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Chemistry Unit 2 > Group 2 > Flashcards

Group 2 Flashcards

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1
Q

What are Group 2 elements also known as?

A

Alkaline earth metals

Their hydroxides exhibit alkaline properties.

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2
Q

What happens to the reactivity of Group 2 elements as you move down the group?

A

Reactivity increases

This trend is related to ionisation energies.

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3
Q

What is a common physical property of Group 2 elements?

A

All are light metals

They are characterized by their low density.

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4
Q

What color are the compounds of Group 2 elements typically?

A

White or colourless

This applies to most of their common compounds.

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5
Q

Do Group 2 elements have high or low melting and boiling points?

A

Reasonably high

They exhibit higher melting and boiling points compared to alkali metals.

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6
Q

What is the electronic configuration of Beryllium?

A

[He]2s2

Beryllium has an atomic number of 4.

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7
Q

What is the electronic configuration of Magnesium?

A

[Ne]3s2

Magnesium has an atomic number of 12.

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8
Q

What is the electronic configuration of Calcium?

A

[Ar]4s2

Calcium has an atomic number of 20.

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9
Q

What is the electronic configuration of Strontium?

A

[Kr]5s2

Strontium has an atomic number of 38.

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10
Q

What is the electronic configuration of Barium?

A

[Xe]6s2

Barium has an atomic number of 56.

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11
Q

What is the electronic configuration of Radium?

A

[Rn]7s2

Radium has an atomic number of 88.

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12
Q

How does the atomic radius change down Group 2?

A

Increases down the group

This is due to the increase in the number of filled shells.

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13
Q

What is the trend in first ionisation energy down Group 2?

A

Decreases down the group

This trend is related to atomic size and electron shielding.

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14
Q

What happens to the density of Group 2 metals down the group?

A

Density increases down the group

Although atomic size increases, the atomic mass increases at a greater rate.

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15
Q

What is the atomic radius of Beryllium in nm?

A

0.3 nm

Beryllium is the smallest in the group.

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16
Q

What is the atomic radius of Magnesium in nm?

A

0.2 nm

Magnesium is larger than Beryllium.

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17
Q

What is the atomic radius of Calcium in nm?

A

0.1 nm

Calcium continues the trend of increasing atomic radius.

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18
Q

What is the atomic radius of Strontium in nm?

A

0 nm

Strontium’s atomic radius increases further.

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19
Q

What is the atomic radius of Barium in nm?

A

0 nm

Barium is larger than Strontium.

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20
Q

What is the atomic radius of Radium in nm?

A

0 nm

Radium has the largest atomic radius in Group 2.

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21
Q

How is the electron configuration for a Group II element obtained?

A

By adding an electron to the electron configuration for the adjacent Group I element

This process involves forming a pair of electrons in the outermost s-type subshell.

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22
Q

Why do electrons in the outermost s-type subshell of a Group II metal experience a greater nuclear charge?

A

Because they are shielded by the same amount as the outermost electron in the adjacent Group I element

This results in the electrons being held more tightly.

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23
Q

What is the trend in size and first ionisation energy of Group II metals compared to Group I metals?

A

A Group II metal is smaller and has a higher first ionisation energy than the adjacent Group I metal

This is due to the increased nuclear charge experienced by the outermost electrons.

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24
Q

What happens to the first ionisation energies of Group II elements down the group?

A

They become smaller

This is due to the outermost electrons being further from the nucleus and better shielded.

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25
What causes the first ionisation energy to decrease as atoms get bigger down the Group II?
The electrons in the outermost s-type subshell become easier to remove ## Footnote This is due to increased distance from the nucleus and increased shielding.
26
How do Group II metal ions compare in size to adjacent Group I metal ions?
Group II metal ions are smaller ## Footnote This is because they have the same electron configuration but the outermost electrons in the Group II ion are more strongly attracted to the nucleus.
27
What do Group II metals form when they react with oxygen?
The corresponding metal oxide ## Footnote This reaction is exothermic and emits visible light characteristic of the metal.
28
What is the nature of the reaction when Group II metals are heated in air?
It is exothermic ## Footnote The metal emits visible light during this reaction.
29
Fill in the blank: The first ionisation energies of the Group II elements become _______ down the group.
smaller
30
True or False: The outermost electrons in Group II metal ions are shielded more than those in Group I metal ions.
False ## Footnote They are shielded by the same amount.
31
What is the reaction of magnesium with oxygen?
2Mg(s) + O2(g) → 2MgO(s) ## Footnote Observations: white powder formed, white flame.
32
What color flames do Group II metals produce when burned in air?
* Calcium: brick red flame * Strontium: crimson flame * Barium: green flame ## Footnote Each metal forms its corresponding oxide when burned.
33
What is the reaction of barium with oxygen?
Ba(s) + O2(g) → BaO2(s) ## Footnote Observations: white powder formed, green flame.
34
What type of compounds do Group II elements form when solid?
White compounds ## Footnote On dissolving in water, they form colorless solutions.
35
What do Group II metals react with to form metal hydroxide and hydrogen gas?
Water ## Footnote The reaction produces a solution of the corresponding metal hydroxide.
36
What is the balanced equation for calcium reacting with cold water?
Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g) ## Footnote The reaction produces hydrogen gas and a solution of calcium hydroxide.
37
What observations occur when calcium reacts with water?
* Fizzing * The mixture warms up * The metal rises and falls, disappearing ## Footnote A white cloud forms due to the calcium hydroxide produced.
38
What happens when Group II metals react with steam?
They form the metal oxide and hydrogen gas. ## Footnote This is a different reaction compared to their reaction with cold water.
39
What equipment is used for heating in the described experiments?
* Crucible * Pipe clay triangle * Tripod * Bunsen burner * Heat resistant mat ## Footnote These are essential for safely conducting reactions involving metals.
40
True or False: The simple compounds of Group II elements are colored when solid.
False ## Footnote They are white when solid.
41
Fill in the blank: The heavier Group II metals in an oxygen-rich atmosphere produce _______.
metal peroxide ## Footnote This is represented as MO2 for the corresponding metal.
42
What gas is produced when Group II metals react with cold water?
Hydrogen gas ## Footnote This reaction also produces a corresponding metal hydroxide.
43
What is the appearance of a saturated solution of calcium hydroxide?
Cloudy white appearance ## Footnote This occurs due to the formation of a suspension of solid calcium hydroxide.
44
What happens to the pH of the solution as magnesium hydroxide is formed?
Gradual increase in pH ## Footnote This is monitored using universal indicator, showing a color change from green to blue.
45
How does the reactivity of Group II metals with cold water change down the group?
Increases, becoming much more vigorous ## Footnote This is demonstrated by the relative rates of reaction of calcium and magnesium.
46
What type of reaction occurs between less reactive Group II metals and steam?
Very exothermic reaction ## Footnote This reaction produces intense white light.
47
What do Group II metals produce when they react with dilute acids?
Hydrogen gas and an aqueous solution of the corresponding metal salt ## Footnote The reactivity increases down the group.
48
Which Group II elements react safely with dilute acids?
Be, Mg, and Ca ## Footnote These are the lighter Group II elements.
49
Complete the reaction: Mg + 2HCl(aq) → _______ + H2(g)
MgCl2(aq) ## Footnote This demonstrates the reaction of magnesium with dilute hydrochloric acid.
50
What is the effect of heating magnesium in the presence of steam?
Produces intense white light ## Footnote This indicates a vigorous reaction.
51
What is the general reaction of magnesium with dilute sulfuric acid?
Mg + H2SO4(aq) → MgSO4(aq) + H2(g) ## Footnote This reaction produces magnesium sulfate and hydrogen gas.
52
What is the general reaction of calcium with dilute nitric acid?
Ca + 2HNO3(aq) → Ca(NO3)2(aq) + H2(g) ## Footnote This reaction produces calcium nitrate and hydrogen gas.
53
True or False: The reactions of dilute nitric acid with Group II metals are straightforward.
False ## Footnote The reactions are complex due to the reduction of nitrogen in nitric acid to gaseous products.
54
What gases are produced when metals react with dilute nitric acid?
Nitrogen(II) oxide (NO) and nitrogen(IV) oxide (NO2) ## Footnote Brown fumes are observed due to the oxidation of NO to NO2.
55
What type of oxides are Group II metal oxides?
Basic oxides ## Footnote Basic oxides act as proton (H+) acceptors.
56
What is the general equation for the reaction of Group II metal oxides with water?
MO + H2O → M(OH)2 ## Footnote This reaction forms a metal hydroxide.
57
Provide an example of a reaction of calcium oxide with water.
CaO + H2O → Ca(OH)2 ## Footnote This results in a colourless solution and heat is released.
58
What are the observations when Group II metal oxides react with water?
Heat is released; the solid expands or crumbles; a colourless solution is formed. ## Footnote Calcium oxide is often studied for this reaction.
59
What products are formed when Group II metal oxides react with dilute mineral acids?
Salt and water ## Footnote The reactions typically require warming and heat is released.
60
Write the general equation for the reaction of a Group II metal oxide with hydrochloric acid.
MO + 2HCl → MCl2 + H2O ## Footnote This demonstrates the basic nature of Group II metal oxides.
61
What is thermal decomposition?
The breaking down of a chemical substance with heat into at least 2 chemical substances. ## Footnote This concept is important for understanding the behavior of Group II carbonates.
62
What happens to Group II carbonates when heated?
They decompose ## Footnote Thermal stability varies among different Group II carbonates.
63
What is charge density?
The magnitude of charge divided by the volume of the ion. ## Footnote Small ions with high charge have higher charge density.
64
Fill in the blank: The thermal stability of a compound refers to its stability to heat and whether it will _______.
decompose on heating ## Footnote This is relevant for understanding the behavior of compounds under heat.
65
What happens to the ease of thermal decomposition of Group 2 carbonates as you go down the group?
The ease of thermal decomposition decreases
66
How does the thermal stability of Group 2 carbonates change down the group?
Group 2 carbonates become more thermally stable down the group
67
What factors influence the thermal stability of Group 2 carbonates?
The charge density of the cation and the ability of the cation to polarise and destabilise the anion
68
What is the effect of cation size on the thermal stability of Group 2 carbonates?
The size of the metal cation increases down the group
69
How does charge density of cations in Group 2 change down the group?
The charge density of the cation decreases down the group
70
Fill in the blank: The carbonate ion, CO₃²⁻, can be polarised and destabilised by a larger charge density of a smaller ion such as _______.
Mg²⁺
71
Which Group 2 ion has a lower charge density, Ba²⁺ or Mg²⁺?
Ba²⁺
72
What is the implication of lower charge density in barium ions on the thermal decomposition of barium carbonate?
Barium carbonate requires more energy to thermally decompose than other Group 2 carbonates
73
What trend is observed in the thermal stability of Group 2 hydroxides?
The thermal stability shows a similar trend to that of the carbonates
74
Why is more energy required to decompose Group 2 hydroxides further down the group?
A larger cation has a lower charge density and is less able to polarise and destabilise the hydroxide ion
75
What is the thermal decomposition reaction of magnesium hydroxide?
Mg(OH)₂(s) → MgO(s) + H₂O(g)
76
What happens to the solubility of Group 2 hydroxides as you go down the group?
The solubility increases ## Footnote This means that more hydroxide ions are formed for the same amounts, leading to increased alkalinity.
77
Which Group 2 hydroxide is insoluble in water?
None; all Group 2 hydroxides are soluble ## Footnote Group 2 hydroxides dissolve in water forming alkaline solutions.
78
Fill in the blank: The solubility of Group 2 sulphates ______ down the group.
decreases
79
Which Group 2 sulphate is soluble in water?
Magnesium Sulphate ## Footnote Barium Sulphate is insoluble in water.
80
What is the trend in alkalinity as you go down Group 2 hydroxides?
Alkalinity increases ## Footnote This is due to the increase in hydroxide ion formation.
81
List the Group 2 hydroxides in order of increasing solubility.
* Mg(OH)2 * Ca(OH)2 * Sr(OH)2 * Ba(OH)2
82
True or False: Barium Sulphate is soluble in water.
False
83
What do Group 2 hydroxides form when they dissolve in water?
Alkaline solutions
84
As you go down Group 2, what trend occurs in the formation of hydroxide ions?
More hydroxide ions are formed
85
What happens to reactivity in Group II elements as you move down the group?
Reactivity increases ## Footnote This trend is observed due to the decreasing ionization energy and increasing atomic size.
86
What is the trend in atomic radius for Group II elements?
Atomic radius increases ## Footnote This is a result of the addition of electron shells as you move down the group.
87
What happens to the first ionisation energy of Group II elements as you go down the group?
First ionisation energy decreases ## Footnote The decrease is due to the increased distance of the outer electrons from the nucleus.
88
How does the solubility of sulphates change down Group II?
Solubility of the sulphates decreases ## Footnote For example, BaSO4 is less soluble than BeSO4.
89
How does the solubility of hydroxides change down Group II?
Solubility of the hydroxides increases ## Footnote For instance, Ba(OH)2 is more soluble than Be(OH)2.
90
What is the trend in thermal stability of carbonates in Group II?
Thermal stability of the carbonates increases ## Footnote This is due to the increasing size of the cation which stabilizes the carbonate ion.
91
What is the chemical formula for calcium carbonate?
CaCO3(s) ## Footnote Calcium carbonate is commonly found in limestone.
92
What is the reaction of calcium carbonate upon strong heating?
CaCO3(s) -> CaO(s) + CO2(g) ## Footnote This decomposition reaction produces quicklime and carbon dioxide.
93
What does quicklime produce when it reacts with water?
Slaked lime (calcium hydroxide) ## Footnote The reaction is represented as CaO(s) + H2O(l) -> Ca(OH)2(s).
94
What is a common use of magnesium oxide?
Used in indigestion remedies ## Footnote It neutralizes excess acid in the stomach, treating heartburn and acid indigestion.
95
In addition to its use in indigestion remedies, where else is calcium carbonate found?
Toothpaste and cement ## Footnote Calcium carbonate is also used in making concrete.

Chemistry Unit 2 (11 decks)

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